Answer:
Rate constant = 0.01238 days⁻¹
Explanation:
The first order reaction has as general equation:
Ln[A] = -kt + Ln[A]₀
<em>Where [A] is concentration of the reactant after time t,</em>
<em>k is rate constant</em>
<em>And [A]₀ the initial concentration of the reactant</em>
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The half-life is the time required to reach the half of the initial concentration. If [A]₀ = 1; [A] = 1/2
Replacing:
Ln[1/2] = -kt + Ln[1]
-0.693 = -k*56days
0.01238days⁻¹ = k
<h3>Rate constant = 0.01238 days⁻¹</h3>
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